Chemistry 1-2E Semester I Study Guide Name Hour Chapter 1 1. Define the following terms. Matter Mass Law of Conservation of Mass 2. Define and give 2 examples of the following: Pure substance Element Compound Mixture Homogeneous Heterogeneous 3. What are the 3 phases of matter? 4. What is a physical change? Give 2 examples. 5. What is a chemical change? Give 2 examples. 6. What is the difference between an endothermic and exothermic reaction?
7. What is a group or family? What do all members of a group have in common? 8. What are the names of the following groups? Group 1 Group 2 Group 17 Group 18 9. How are group 18 elements different than all other elements? 10. Where are the following found on the periodic table? Metals Nonmetals Metalloids Transition metals 11. List properties of metals, nonmetals and metalloids. 12. Are most elements metals, nonmetals, or metalloids? What state do most elements exist in at room temperature? 13. What is a period? How many are there on the periodic table? 14. What happens to atoms in chemical reactions? Chapter 2 15. How are quantitative observations different than qualitative observations? Give 2 examples of each
16. How many significant figures are there in each of the following numbers? a. 27 b. 2700 c. 2700. d. 2700.0 e. 2.7 x 10 3 f. 0.0524 g. 0.05240 h. 5.24 x 10-1 i. 5.240 x 10-2 17. Give the result of each of the following calculations in the correct number of significant figures. a. 124.0 x 2.4 = b. 1.240 x 10 2 x 2.4 = c. 83 + 55.89 + 72 = d. 123.4 + 0.06 + 100.0 = e. 123.4-0.06 + 100.0 = 18. Complete the following chart for SI prefixes: 1 g = mg 1 kg = g 1 g = cg 19. Convert the following measurements: a) 1200 cm = m 675 ml = L b) 4.8 kg = g 0.004 g = mg c) 20 m = mm 20. Distinguish between mass and weight. 21. What is the formula for density? 22. Define weight and explain how it changes as gravity changes. 23. Calculate the density of an object with a mass of 2.34 g and a volume of 4.68 ml.
24. A graduated cylinder has 20 ml (cm 3 ) of water placed in it. An irregularly shaped rock is then dropped in the graduated cylinder and the volume of the rock and water in the cylinder now reads 30 ml (cm 3 ). The mass of the rock dropped into the graduated cylinder is 23 grams. a. Find the volume of the rock dropped into the graduated cylinder. b. Find the density of the rock dropped into the graduated cylinder. 25. Explain the difference between accuracy and precision and give an example of each. 26. List the SI base unit for mass, volume, length, time, amount of substance, and temperature. Chapter 3 27. What are the charges of the 3 subatomic particles? 28. What is an isotope? Give an example 29. Fill in the chart below for the following neutral atoms. Element Atomic # Mass # # of protons # of electrons # of neutrons P-32 Ca-40 Br-81 I-125 Au-197 30. How many valence electrons do the following have? K Mg Al C P O Br Ar
31. How many valence electrons do most atoms need to become as stable as possible? 32. What part of the atom is involved in compound formation? 33. Why don t noble gases react with other substances? 34. Define the following: ion, anion, and cation. 35. Summarize Rutherford s conclusions from his gold foil experiment. 36. Calculate the average atomic mass of magnesium using the following data for three magnesium isotopes. Isotope mass (u) relative abundance Mg-24 23.985 78.7% Mg-25 24.986 10.13% Mg-26 25.983 11.17% Chapter 4 37. What is a wavelength? 38. Which color on the electromagnetic spectrum have the longest and shortest wavelength? 39. How does an atom move from the ground state to the excited state? 40. Fill in the following chart: Main energy level Sublevels in main energy levels Number of orbitals/sublevel Number of orbitals/main level Number of electrons/sublevel Number of electrons/main level
41. Write the electron configuration for: a. Phosphorus b. Arsenic 42. Write the noble gas shortcut electron configuration for calcium. Chapter 5 43. Whose idea was it to arrange the elements in the periodic table according to their chemical and physical properties? 44. Why did Mendeleev leave empty spaces in his periodic table? 45. What scientists work led to a periodic table based on increasing atomic number? 46. Write the name of the following groups of elements: Group 1 Group 2 Group 17 Group 18 47. Write the name of the elements with atomic numbers from: 58 to 71 90 to 103 48. Define the following terms as they relate to the periodic table: Group Period 50. Indicate the number of valence (outermost) the following elements have: K C Cl Mg P Ar Al S 52. What is the main characteristic of noble gases?
53. Which are more reactive, alkali metals or alkaline-earth metals? Why? 54. Define the term electronegativity. Which elements have a high and low electronegativity? What is the general trend on the periodic table? 55. Define the term ionization energy. Which elements have a high and low ionization energy? What is the general trend on the periodic table? 56. How does atomic radius change as you move across a row and down a group on the periodic table? 57. Define the terms anion and cation. Give an example of each. Chapter 6 58. Which electrons are involved in the formation of a chemical bond 59. What is the difference between a polar covalent and a nonpolar covalent bond? 60. What is the difference between an ionic and a covalent bond? 61. What subatomic particles are shared in a covalent bond? 62. What is a molecule? 63. What does the octet rule state?
64. What do you need to know before you draw a Lewis structure (dot diagram). 65. After you finish drawing a Lewis structure, what should you double check? 66. Draw Lewis structures and use VSEPR theory to predict the shapes (with bond angles) for the following: NH 3 CH 4 OH - H 2 O 67. What is a hybrid orbital? What type of hybrid orbitals would CCl 4 have? 68. What term is used to describe the movement of electrons involved in a metallic bond? 69. Define the following terms: Ductile Malleable
Chapter 7 70. Write the formula for the following ionic compounds. a. calcium iodide b. sodium chloride c. lead (II) sulfide d. magnesium fluoride e. iron (III) carbonate lithium nitrate g. aluminum hydroxide 71. Name the following ionic compounds. a. Al 2 O 3 b. K 2 O c. FeCl 2 d. Na 2 CO 3 e. Mg(NO 3 ) 2 f. Cu 2 SO 4 h. Mg 3 (PO4) 2 72. Indicate the prefixes used for covalent names for the following: 1 6 2 7 3 8 4 9 5 10 73. Write the formula for the following binary molecular (covalent) compounds. a. phosphorus trichloride carbon dioxide c. phosphorus tetraoxide dinitrogen pentoxide e. silicon dioxide 74. Name the following binary molecular substances. a. SO 2 CO b. SO 3 CF 4 c. IF 7
75. Write the formula and charge of the following polyatomic ions. a. ammonium nitrite b. nitrate hydroxide c. carbonate sulfate d. phosphate 76. Name the following acids a. HCl HF b. H 2 SO 4 H 3 PO 3 77. Write the formula for the following acids. a. Hydrosulfuric acid Hydrobromic acid b. Carbonic acid Nitrous acid 78. What is Avogadro s constant? What does it mean? 79. Define the term molar mass. 80. Determine the molar mass of the following: a. CO 2 b. H 2 SO 3 c. Mg(NO 3 ) 2 81. How many atoms are in 4.67g of zinc? 82. What is the number of moles represented by 25.6 g of CaCl 2?
83. What is the mass of 3.45 moles of Al 2 (SO 4 ) 3? 84. What is the mass of 14.2 L of carbon dioxide gas? 85. What is the percent composition of each element in Al 2 (CO 3 ) 3? 86. What s the empirical formula of a molecule containing 65.5% carbon, 5.5% hydrogen, and 29.0% oxygen? 87. If the molar mass of the compound in problem 61 is 110 grams/mole, what s the molecular formula? 88. In an experiment, rubidium chloride hydrate was heated to remove water. The following data was obtained: 1. Mass of empty crucible 60.286 g 2. Mass of crucible & contents before heating 79.376 g 3. Mass of crucible & contents after heating 70.366 g 4. Calculate: a) The formula of the hydrate: b) The name of the hydrate: c) The percent water of the compound